HARRY S TRUMAN COLLEGE One of the City Colleges of Chicago. Course Syllabus Spring 2014

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1 HARRY S TRUMAN COLLEGE One of the City Colleges of Chicago Course Syllabus Spring 2014 Course Title and Section: CHEMISTRY 201 Section DEN Length of Course: 16 weeks Credit Hours: 5 Contact Hours: 8 Class Meeting Times: 1:00-4:50 pm MW Room: 3831 Instructor: Prof. James Czuchra jczuchra@ccc.edu Phone: (773) Office: 3826A or check in classroom 3831 during office hours Office Hours: 12:00-12:50 pm MW Course Website: It is required that you check this website regularly for announcements, problem sets, and lab activities. Also check your CCC account regularly. Online homework at To register, you need your address, the course ID (CZUCHRA96118), and the access code (usually on a card purchased with the book). Truman College Mission Statement: Our Mission dedicates us to deliver high-quality, innovative, affordable, and accessible educational opportunities and services that prepare students for a rapidly changing and diverse global economy. Truman College General Education Goals: The student exhibits social and ethical responsibility and is aware of her or his place in the global community. The student performs effectively in the workplace and has the ability to work and make effective use of a wide variety of current technologies. The student communicates effectively in both written and oral formats. The student demonstrates the ability to think critically, abstractly, and logically. The student gathers interprets and analyzes data. Course Description and Prerequisites: CHEMISTRY 201: General Chemistry I Topics include the periodic table of the elements, atomic structure, basic concepts of quantum theory, bonding, stoichiometry of compounds and reactions, thermochemistry, the gaseous state, basic concepts of the liquid and solid states, solutions, acids and bases. Writing assignments, as appropriate to discipline, are part of the course. Prerequisite: Eligibility for Mathematics 140 or higher and Grade of C or better in Chemistry 121 or one year of high school chemistry, or Consent of Department Chairperson. 4 lecture and 4 lab hours per week. 5 credit hours. 1

2 Required Text and Materials: Text: Chemistry: A Molecular Approach, Third Edition, by Nivaldo J. Tro, An all chapter version if you plan on continuing to CHEM 203 is ISBN If you will NOT be taking CHEM 203, you may use a shorter version containing just the first 12 chapters. It's ISBN is Materials: notebook, composition book (see in class), pen, scientific calculator (cell phones and other devices not permitted on quizzes or tests) Students Course is Expected to Serve: The course is intended for students pursuing degrees in chemistry, pharmacology, biology, engineering, nursing, and premed. Course Objectives: At the completion of this course, the successful student will be able to: Solve quantitative chemistry problems and demonstrate reasoning clearly and completely. Integrate multiple ideas in the problem solving process. Describe, explain and model chemical and physical processes at the molecular level in order to explain macroscopic properties. Classify matter by its state and bonding behavior using the Periodic Table as a reference. Apply important theories such as the Kinetic Molecular Theory of Gases or the Quantum Mechanical Theory of the Atom to the solution of general chemistry problems. Perform general chemistry laboratory experiments using standard chemistry glassware and equipment and demonstrate appropriate safety procedures. Record, graph, chart and interpret data obtained from experimentation and use that information to correctly identify/analyze assigned unknown substances. Measureable Student Learning Outcomes: The (R) designation means this is a review topic-- something from Chemistry 121. As such, we will cover these topics more rapidly. At the completion of this course, the successful student will be able to: Scientific Method (R) Describe the scientific method. (R) Define and explain the terms: law, hypothesis, and theory. Chemical Calculations (R) Use exponential notation. (R) Do mathematical calculations involving significant figures. (R) Differentiate between mass and weight. (R) Convert from the English system to the metric system (& vice versa) common units of length, mass, volume, and temperature. (R) Use the metric system in calculations. Heat and Temperature (R) Differentiate between heat and temperature. (R) Do simple calculations of heat changes using specific heat. Define and use the terms standard state, standard enthalpy change, molar enthalpy of formation. 2

3 Density (R) Solve problems using density as the relationship between mass and volume. Properties of Matter (R) Use and define (describe or explain) basic chemical concepts with respect to properties of matter: physical states of matter, physical and chemical properties of matter, physical and chemical changes, the law of conservation of mass, the law of conservation of energy, the law of definite composition, classification of elements. (R) Distinguish between pure substances (elements and compounds) and mixtures (homogeneous and heterogeneous). List the names and chemical symbols of at least 48 elements. Atomic Theory and Structure, Molecular Theory and Structure (R) Distinguish between ionic and molecular compounds. (R) Determine the number and types of atoms represented in a chemical formula. Use basic chemical nomenclature for inorganic compounds. Write the formulas of binary ionic compounds, common binary molecular compounds, and at least 12 common acids, 4 common bases, inorganic ternary compounds using 15 common polyatomic ions. Use oxidation numbers to distinguish oxidation states of metals in compounds. (R) Balance chemical equations given the formulas of the reactants and products. Calculate the oxidation number of each element, given the formulas of the reactants and products. Balance redox equations using oxidation numbers. (R) List the basic principles of Dalton's atomic theory and indicate how the theory has been further developed in this century. (R) State the basic properties of the subatomic particles: protons, neutrons, and electrons. (R) Describe the Rutherford atom. (R) Define atomic number, mass number, and isotopes. (R) Define the atomic mass unit and Avogadro's number. (R) Use the conversion factor from grams to amu in simple calculations. Calculate the average atomic mass from isotopic masses and percent abundances. (R) Apply the terms: metals, nonmetals, alkali metals, alkaline earth metals, metalloids, transition metals, noble gases, halogens, and inner transition metals to the arrangement of elements in the periodic table. (R) Describe the arrangement of the elements in the periodic table. (R) Use the periodic table to predict formulas of compounds. (R) Define the terms anion, cation, and polyatomic ion. Describe how ionic and covalent bonds are formed. Calculate the oxidation number of each element in a chemical formula. Mole-Mass Calculations (R) Calculate the percent composition of compounds, given the formulas. (R) Calculate the empirical formula, given the percent composition. (R)Calculate the empirical formula of compound given the mass of the sample, the mass of CO 2 and mass of H 2O produced in a combustion reaction. (R) Distinguish between empirical and molecular formulas. (R) Explain the concepts of the chemical quantity, the mole, and relate it to counting of atoms and molecules. (R) Convert mass in grams to moles, formula units, molecules (and/or atoms) using atomic weights, formula weights, and molecular weights. 3

4 List the basic rules which predict whether a salt is soluble in water. Stoichiometry Write the balanced equations describing several examples of combustion, acid-base, precipitation, and exchange reactions. Write the equations in the molecular, total ionic and net ionic format. (R) Explain the information given by the balanced chemical equations. Perform stoichiometric calculations from a given chemical equation. Use calculations determine the limiting reagent, how much excess reagent is left, and the theoretical and percentage yield of each product. Solutions List the properties of solutions and distinguish true solutions from heterogeneous and colloidal mixtures. Define solubility, percent concentration, molarity, mole fraction, and molality. Explain factors affecting solubility and the rate of dissolving. Write molecular, total ionic and net ionic equations which show that the solution is the reaction medium. Use percent concentration, molarity, and molality in stoichiometric calculations. Gases List the basic principles of the Kinetic Molecular Theory of gases. (R) Describe the measurement of pressure using a barometer. (R) Use four kinds of pressure units in calculations and convert from one to another. Calculate pressure, volumes, and temperatures of gases using Boyle's law, Charles' Law, the Combined Gas Law, and Dalton's Law of Partial Pressures. (R) Calculate Kelvin temperatures from Centigrade and vice versa. (R) Define standard conditions of temperature and pressure. Use the Ideal Gas Law to calculate density and molecular weight of a gas. Use the gas laws in chemical stoichiometric calculations. Define and distinguish between diffusion and effusion. Energy and Light Define and explain the terms electromagnetic radiation, wavelength, frequency, wave amplitude, spectrum, and nodes. Describe the Bohr hydrogen atom; describe the hydrogen atom in terms of simple quantum mechanics. Perform calculations using the equation λν = c. Explain the source of the atomic line spectra. Describe the properties of light. Molecular Orbital Theory Write electronic configurations of the first 50 elements; show the diagrams of their electronic structure, and indicate the spin of each electron. Sketch the shape of the s, p and d orbitals. Identify the 4 quantum numbers for any electron in an atom. Predict which atoms or ions are paramagnetic and which are diamagnetic using the electronic configurations. State the Pauli Exclusion Principle, Hund's rule, and the Aufbau principle. 4

5 (R) Define ionization energy and be able to rank using the periodic table. Use ionization energy trends to predict the stability of electronic configurations and the tendency for outer shell electrons to undergo changes in order to form compounds. (R) Define electronegativity: show how it varies with respect to the periodic table. (R) Use electronegativity to estimate the polarity of bonds. Show the trends of atomic and ionic sizes on the periodic table. State the octet rule, including exclusions. Write Lewis electron dot structures for simple covalent compounds and polyatomic ions. Use double and triple bonds to show structures of molecules and ions; use resonance to describe equivalent bonds. Use the Valence Shell Electron Pair Repulsion theory to describe electron pairs geometry, molecular geometry, hybridization, and bond angles. Predict the polarity of bonds and molecules. Define bond order and bond dissociation energy; use bond energies to estimate reaction enthalpies. Calculate the formal change of an atom in a molecule or ion, and use it to predict the most reasonable resonance structures. Explain the difference between oxidation number and formal change. Explain simple valence bond theory. Use the concepts of orbital overlap, sigma and pi bonds, hybrid orbitals to explain the strength and orientation of covalent bonds. Properties of Solutions Use molarity in calculations concerning the dilution of solutions. Explain at least two examples of colligative properties. Calculate the freezing point depression and the boiling point elevation due to the addition of a nonvolatile molecular solute to a pure solvent. Acids and Bases List at least four properties each for acids and bases. Explain the behavior of acids and bases in terms of the Arrhenius and Brønsted/Lowry theories. Write equations for acids and bases showing conjugated acid/base pairs. List at least five common strong acids and five common strong bases. Given an acid, write the formula of the conjugate base, and vice versa. Write complete equations for at least two examples of each of the following reactions: acid + base, acid + metal, acid + metal oxide, acid + carbonate. Given the formula of a salt, write the formulas of the acid and the base which would react to form the salt. Distinguish between electrolytes and non-electrolytes, strong and weak electrolytes. List at least three examples of each. Define ph. Given a ph value, state whether the solution is acidic, basic, or neutral. Given a ph value calculate the H + concentration, and vice versa. Estimate ph and poh values without the use of a calculator given H + concentration and/or OH - concentration. Given a poh value calculate the OH - concentration, and vice versa. Convert from H 3O + concentration to ph then to poh then to OH - concentration. Laboratory and Evaluations Perform simple tasks in the laboratory. Carry out laboratory measurements and calculations using the correct significant figures. Perform the necessary calculations, prepare any required graphs and answer the questions for each experiment. 5

6 Achieve a grade of at least 50% for the final comprehensive examination. Record all data in ink directly onto the data sheet or in the laboratory notebook. Prepare a lab report including a summary. On any quizzes and exams, answer short essay questions. Methods of Instruction: Lecture, lab, demonstrations, classwork, discussions Definition / Statement of Active Pursuit of the Course: Students who do not meet basic, instructordefined criteria for active pursuit may receive an ADW (administrative withdrawal) at midterm. Lack of active pursuit is defined as more than 2 absences, 4 tardies, or failure to turn in 2 or more labs by midterm. District and College attendance policies are listed in the college catalog and the Student Policy Manual: No Show Policy: If a student registered for the course before the start time of the first class period, but did not attend either of the first two classes (or the first class only for once-a-week courses), the instructor will report it on the Day 10 class lists and Registrar s Office will remove the student from the course. Academic integrity: The City Colleges of Chicago is committed to the ideals of truth and honesty. In view of this, students are expected to adhere to high standards of honesty in their academic endeavor. Plagiarism and cheating of any kind are serious violations of these standards and will result, minimally, in the grade of F by the instructor. Check out the Student Policy Manual, page 44, for the District s policy on academic honesty: Student Conduct: City Colleges of Chicago students are expected to conduct themselves in a manner which is considerate of the rights of others and which will not impair the educational mission of the College. Misconduct for which students are subject to College Discipline (e.g. expulsion) may include the following: (1) all forms of dishonesty such as stealing, forgery, (2) obstruction or disruption of teaching, research, administration, disciplinary proceeding, (3) physical or verbal abuse, threats, intimidation, harassment, and/or other conduct that threatens or endangers the health or safety of any person, and (4) carrying or possession of weapons, ammunition or other explosives. Check out the Student Policy Manual, above, for more information. Disability Access Center: Any student with a disability, including a temporary disability, is eligible for reasonable accommodations and should contact the Disability Access Center located in room 1428 as soon as possible. Instructors can only honor accommodation requests from the DAC. Classroom Etiquette: I want every student to be successful in learning chemistry. You came here to learn but distractions hinder the learning process for you and your classmates. Please turn off all cell phones while in class. Do not text or listen to music while in class. When a general question is posed to the class, please do not blurt out an answer raise your hand. I want every student to have the chance to think about the question before the answer is revealed. Lab safety is very important. Not following safety rules will result in being asked to leave the lab and receiving a zero for the activity we are working on. The work you do must be your own. Submitting work that is not your own may result in a grade of F being assigned as a final course grade. Class time is our collective learning time, therefore please understand if you are asked to see me outside of class to pursue questions that are do not advance the planned lesson. Food and drink are prohibited in the classroom and lab. You may quietly leave the room to use the restroom-- no permission required. Children or other guests are not allowed. 6

7 Grading: Your Grade will be based on laboratory reports (lowest one will be dropped) (30%), regular examinations (best two of three) (20%), quizzes (lowest one will be dropped) (20%), a comprehensive final exam which everyone must take (20%), class participation/attendance (5%) and homework (5%). The final exam consists of two parts. One part is the American Chemical Society examination and the other part is instructor made. In general, it's important to understand that A is earned for superior performance, B for good, C for adequate, D for minimal, and F for insufficient. Letter grades are translated to a numerical score for gradebook recording. Midterm and final grades are assigned based on the percentages earned as follows: %, A; 80-89% B; 70-79% C; 60-69%, D, below 60%, F. Late Work and Make-up Policies: Coming to class every day on time is essential to your success in this class. Quizzes are given at the beginning of the class session. There are no make ups of any missed work. One participation point will be deducted for every absence beyond the first two or every 2 tardies beyond the first two. Leaving early and extended breaks will be counted as a tardy. Grades are cumulative (NOT the average of midterm and second quarter grades). Late work may be turned in for partial credit (typically 50%) up to a week after its due date. Topical Outline/Course Calendar: See the attached calendar for important dates including course topics and laboratory activities. 7

8 . Chem 201 DEN M 1:00 4:40 Room 3831 W 1:00 4:40 Room 3831 January/February 2014 Monday Tuesday Wednesday Thursday Jan Mr. James Czuchra February/March 2014 Monday Tuesday Wednesday Thursday Feb Course overview Topic A Topic A, B Lab 0 Topic F Topic F, G Lab Mar ML King Holiday Topic B Lab 1 Topic G Topic G, H Lab Topic B, C Topic C Lab 2 Topic H Topic I Midterm Exam 2 Feb Topic C, D Topic D Lab 3 Topic I, J Lab 7 Topic J Topic E Topic E Exam 1 Topic K Lab 8 Topic K 17 President s Day Holiday Topic F Lab 4 A Scientific Method, Measurement, and Problem Solving (Ch. 1) B Atomic Theory, Elements, Atomic mass, and the Mole (Ch. 2) C Compounds: Composition, Nomenclature, and Equations (Ch. 3) D Stoichiometry, Reaction Types, and Oxidation States (Ch. 4) 20 E Reactions in Aqueous Solutions (Ch. 4) F Gas Behavior (Ch. 5) G Thermochemistry (Ch. 6) H Atomic Theory continued (Ch. 7) I Periodicity (Ch. 8) J Chemical Bonding Basics (Ch. 9) K Chemical Bonding continued (Ch. 10) L Intermolecular Forces: Liquids & Solids (Ch. 11) M Solutions and Their Physical Properties (Ch. 12) N Acids & Bases (Ch. 15 or class notes)

9 Chem 201 DEN M 1:00 4:40 Room 3831 W 1:00 4:40 Room 3831 April 2014 Monday Tuesday Wednesday ThursdaMar Mar Mr. James Czuchra May 2014 Monday Tuesday Wednesday Thursday Topic L Lab 9 7 Last day to withdraw Topic M Lab Spring Break 21 Topic M Spring Break Topic L Exam 3 Topic M Spring Break Topic N Lab Spring Break 24 Lab Check Out Loose Ends Final Exam Review LAST CLASS Final Exam Lab 0 Check-In Lab 1 Simple Qualitative Analysis Lab 2 Quantitative Analysis of a Mixture Lab 3 Single & Double Displacement Reactions Lab 4 Qualitative Analysis Lab 5 Molar Mass of a Volatile Liquid Lab 6 Calorimetry Lab 7 Atomic spectra Lab 8 Periodicity (half lab) Lab 9 Molecular Geometry Lab 10 Chromatography (half lab) Lab 11 Freezing Point Depression Lab 12 - Neutralization/Titration 28 Topic N Lab Topic N May 1 Note: This schedule, including the list of topics and lab experiments, is subject to change. J Chemical Bonding Basics (Ch. 9) K Chemical Bonding continued (Ch. 10) L Intermolecular Forces: Liquids & Solids (Ch. 11) M Solutions and Their Physical Properties (Ch. 12) N Acids & Bases (Ch. 15 or class notes)